The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given rG- - A - BT- where A and B are non-zero constants- Which of the following is true about this reaction-

We know the relation G^∘ = H^∘ T S^∘ Given that A and B are non zero constants, i.e., nbsp; A = H^∘ , B = S^∘ if H^∘ is positive means reaction is endot ...

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Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

The standard ...

Question

The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given $△_{r} G^{\circ} = A - B T,$ where A and B are non-zero constants. Which of the following is true about this reaction?

Exothermic if A > 0 and B < 0

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Endothermic if A < 0 and B > 0

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Endothermic if A > 0

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Exothermic if B < 0

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Solution

The correct option is C Endothermic if A > 0
We know the relation $△ G^{\circ} = △ H^{\circ} - T △ S^{\circ}$
Given that A and B are non-zero constants, i.e.,
$A = △ H^{\circ}, B = △ S^{\circ}$
if $△ H^{\circ}$ is positive means reaction is endothermic.

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Similar questions

Q. The standard reaction Gibbs energy for a chemical reaction at an absolute temperature

T

is given by:

Δ_{r} G^{o} = A - B T

Where

A

and

B

are non-zero constants. Which of the following is true about this reaction?

Q. The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by,

Δ_{r} G^{o} = A - B T

Where A and B are non-zero constants.
Which of the following is true about this reaction?

Q. The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given

△_{r} G^{\circ} = A - B T,

where A and B are non-zero constants. Which of the following is true about this reaction?

ASSERTION(A): For every chemical reaction at equilibrium, standard Gibbs energy of the reaction is zero.
REASON(R): At constant temperature and pressure, chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.

Q. Assertion: For every chemical reaction at equilibrium, the standard Gibbs energy of reaction is zero.
Reason: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

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The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given △rG∘=A−BT, where A and B are non-zero constants. Which of the following is true about this reaction?

The correct option is C Endothermic if A > 0We know the relation △G∘=△H∘−T△S∘ Given that A and B are non-zero constants, i.e., A=△H∘,B=△S∘ if △H∘ is positive means reaction is endothermic.

The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given $△_{r} G^{\circ} = A - B T,$ where A and B are non-zero constants. Which of the following is true about this reaction?

The correct option is C Endothermic if A > 0
We know the relation $△ G^{\circ} = △ H^{\circ} - T △ S^{\circ}$
Given that A and B are non-zero constants, i.e.,
$A = △ H^{\circ}, B = △ S^{\circ}$
if $△ H^{\circ}$ is positive means reaction is endothermic.